2.1.1 Ordering Metals by Reactivity

• The reactivity series is a list of metals ordered from most to least reactive
• Name three common metals found in the reactivity series.

  Potassium, Sodium, Calcium
• What are four factors that affect metal reactivity?

  Ionization energy, atomic size, electronic configuration, electronegativity
• What is the purpose of the reactivity series?

  To predict displacement reactions
• The most reactive metals in the series are located at the top
• Factors affecting metal reactivity include ionization energy, atomic size, electronic configuration, and electronegativity
• The reactivity series orders metals from most to least
• What property determines the relative reactivity of metals in the series?

  Electronegativity
• Metals with lower ionization energy are more reactive.


  True
• What does lower electronegativity indicate about a metal's reactivity?

  Weaker electron pull
• Order the metals based on their reactivity in displacement reactions:

  1️⃣ Zinc

  2️⃣ Copper

  3️⃣ Silver

  4️⃣ Gold
• More reactive metals can displace less reactive metals from their compounds.


  True
• Zinc can displace copper, silver, and gold from their compounds.


  True
• What is the reactivity series of metals based on?

  Their ability to displace other metals
• Order the following metals from most reactive to least reactive based on their position in the reactivity series:

  1️⃣ Potassium

  2️⃣ Sodium

  3️⃣ Calcium

  4️⃣ Magnesium

  5️⃣ Aluminum
• Lower electronegativity in metals leads to higher reactivity.

  True
• Stable electronic configurations make metals less reactive.


  True
• What property is related to the order of metals in the reactivity series?

  Electronegativity
• Which factor indicates that a metal is more likely to lose electrons?

  Lower electronegativity
• What does zinc displace copper from in a displacement reaction?

  Copper sulfate solution
• Match the metal with its reactivity level:

  Calcium ↔️ High

  Magnesium ↔️ Medium

  Copper ↔️ Low
• Factors affecting metal reactivity include ionization energy, atomic size, electronic configuration, and electronegativity
• Metals with stable electronic configurations are less likely to lose electrons due to their high stability
• Displacement reactions are used to determine the order of metals in the reactivity series.
• Zinc can displace copper from copper sulfate because it is higher in the reactivity series.
• Potassium can displace all other metals listed in the reactivity series.
• Order the following metals based on their ability to be displaced by zinc:

  1️⃣ Copper

  2️⃣ Silver

  3️⃣ Gold
• Metals with lower electronegativity are more reactive.


  True
• The most reactive metals in the reactivity series are potassium, sodium, and calcium.
• Lower ionization energy means it takes less energy to lose electrons
• The reactivity series is related to the electronegativity of metals, where lower electronegativity indicates higher reactivity
• Metals with lower electronegativity are more reactive.

  True
• More reactive metals can displace less reactive metals from their compounds.


  True
• Metals with lower electronegativity are more likely to form positive ions.


  True
• What property of metals is related to their ability to lose electrons?

  Electronegativity
• Why does a larger atomic size increase metal reactivity?

  Reduces nuclear attraction
• Match the factor with its influence on reactivity:

  Ionization Energy ↔️ Higher reactivity with lower energy

  Atomic Size ↔️ Higher reactivity with larger size

  Electronic Configuration ↔️ High stability leads to lower reactivity

  Electronegativity ↔️ Higher reactivity with lower electronegativity
• Which metal can zinc displace from its compound?

  Copper
• Which metal has the highest reactivity in the series provided?

  Potassium
• Which metal cannot be displaced by copper from its compounds?

  Silver